Question

A hot lump of 35.6 g of copper at an initial temperature of 86.3 C is placed in 50.0 mL initially at 25.0 °C and allowed to reach thermal equilibrium. What is the final temperature of the copper and water, given that the specific heat of copper is 0.385 J/(gxC). Assume no heat is lost to surroundings.

Answer 1

Date O 'heat gain by water - - heat lost by Copper water - copper q=COT me amount of substance (= ' Specific heat of Substance DT = To - T , ; change in temperatur Volume of water is 50.0mL and density of water is 1 glml Density – amount volume amount = Density x volume = 1 X 5070 = 500 g. 500 g X 4. 184 IX (To -25°C) = -35.6 x 0.385 209. 2 I (T2 -25°C) = - 13.7 X (T - 86.2) X (T₂-863 20912 Ty - 5230 = -13 17 T t 1182 go

209.2 Ty + (3 7 T = 1182 +5230 2234 12 6412 12 = 6412 = 28.8°C 223 The kenal temperature of the Copper and water is 28.8 .